Chemistry, 29.07.2019 08:00 lbelle

Explain in terms of collision theory, how and why a reactions's rate changes as the reaction progresses

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The rate of a chemical reaction is the speed with which the reactants are converted to products while the collision theory is used to explain why chemical reactions occur at different rates. It states that for a reaction to proceed, the reactants particles must collide and the more successful collisions there are per unit of time, the faster the reaction will be. As the reaction progresses, the products builds up in the system and the chance that the reactants will collide amongst themselves reduces as the product molecules begin to build up while the molecules of the reactants are deprived. therefore the rate of reaction changes.

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Explanation:

According to collision theory, more is the number of collisions occurring between the combining substances more will be the rate of reaction.

Factors that affect rate of a reaction are as follows.

Temperature - Increase in temperature leads to increase in kinetic energy of particles due to which there occurs more number of collisions between them. As a result, rate of reaction will increase leading to increase in rapid formation of products.

Surface area - More is the surface area of a substance, less will be the interaction between solute and solvent particles. And, when there occurs decrease in surface area then interaction between solute and solvent particles increases. This leads to increase in rate of reaction.

Concentration of reactants - More is the concentration of reactant molecules more is the availability of molecule interaction. As a result, more number of collisions occur leading to increase in rate of a reaction.

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Explain in terms of collision theory, how and why a reactions's rate changes as the reaction progres...